test 3 review
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Test 3 Review. Electric charge. Mass #. Na. # of atoms. Atomic #. Ionic Compounds. Also referred to as a “salt” Formation involves a transfer of electrons Usually made up of a metal and a non-metal Are good conductors when they can be melted or dissolved - PowerPoint PPT PresentationTRANSCRIPT
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Test 3 Review
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NaMass #
Atomic #
Electric charge
# of atoms
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Also referred to as a “salt”
Formation involves a transfer of electrons
Usually made up of a metal and a non-metal
Are good conductors when they can be melted or dissolved
Typically have extremely high melting points
Ionic Compounds
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Formation of an Ionic Bond
Electron acceptor (Cl)
meetselectron donor
(Na)
Ions attract to
form a neutral
pair
e- jumps from Na to Cl
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Smallest building blocks are ions, NOT MOLECULES
Large numbers of ions can attract to form clusters and eventually crystals
Structure
Ion pair Ion cluster Crystal
lattice
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Cations – positively charged ions◦ Na+ Ca2+ Al3+
Anions – negatively charged ions◦ Cl- O2-
Polyatomic ions – ions made up of more than one type of atom◦ NO3
- SO4-2 PO4
-3
Ions
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The number of e- gained, lost or shared ub compound formations◦ Alkali metals +1◦ Alkaline earth metals +2◦ Oxygen group -2◦ Halogens -1
Oxidation Number
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K+ and N3-
◦ K3N
Ca2+ and N3-
◦ Ca3N2
Ba2+ and NO3-
◦ Ba(NO3)2
Criss-cross rule
Write the formulas – ALWAYS put cation first
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Binary – made of 2 ions
Write cation first Change anion ending to –ide
Na+ and Cl-◦ Sodium chloride
H+ and F-
◦ Hydrogen fluoride
CaBr2◦ Calcium bromide
Naming Binary Ionic Compounds
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Name the cation Polyatomic ion name is unchanged
NaNO3◦ Sodium nitrate
Zinc carbonate◦ ZnCO3
Naming Polyatomic Ionic Compounds
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Also called covalent compounds
A molecule is a neutral group of atoms that are held together by covalent bonds
The valence e- are shared by the atoms
Covalent bonding usually occurs between 2 non-metals◦ H2O, CO2, O2, NO
Molecular Compounds
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Naming Molecular Compounds Use prefixes 1 mono-
2 di-3 tri-4 tetra-5 penta-6 hexa-7 hepta-8 octa-9 nona-10 deca-
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P4O10
N2O3
As2O5
OF2
ExamplesTetraphosphorous decoxide
Dinitrogen trioxide
Diarsenic pentoxide
Oxygen difluoride
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H2O2N2Cl2Br2 I2F2
Diatomic Molecules 7 diatomic molecules No noble gases Halogens and N, O, H They are all gases (not
noble gases) except for Br and I
“Honcl brif”
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H2SO4
HF
H3PO4
H2SO3
H2CO3
HNO3
Try these. . .Sulfuric AcidHydrofluoric AcidPhosphoric Acid
Sulfurous Acid
Carbonic Acid
Nitric Acid
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More Practice. . . Calcium bromide
Chromium (III) acetate
Barium sulfate
Copper (I) sulfide
Sulfur hexafluoride
CaBr2
Cr(C2H3O2)3
BaSO4
Cu2SSF6
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Cr2(C2O4)3
Hg(CN)2
Cu(ClO4)2
ZnC4H4O6
More Practice. . . Chromium (III) oxalateMercury (II) cyanide
Copper (II) perchlorateZinc tartrate
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The mass of a compound
In order to calculate molar mass (also called molecular weight) you add up the masses of each element in the compound◦ Be aware of subscript numbers that designate the
amount of atoms per element
You get the masses from the periodic table
**be careful when rounding the mass
How to Calculate Molar Mass
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NaCl◦ Na = 23 g/mol◦ Cl = 35.5 g/mol
H2O◦ H = 1 g/mol (but there are 2) = 2 g/mol◦ O = 16 g/mol
HNO3◦ H = 1 g/mol◦ N = 14 g/mol◦ O = 16 g/mol (but there are 3) = 48 g/mol
Ba(NO3)2◦ Ba = 137.3 g/mol◦ N = 14 g/mol (but there are 2) = 28 g/mol◦ O = 16 g/mol (but there are 6) = 96 g/mol
Examples 58.5 g/mol
18 g/mol
63 g/mol
261.3 g/mol
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All metal atoms in a metallic solid contribute their valence e- to form a “sea” of e-◦ These e- move easily and freely because they are
not tied to a specific atom Delocalized electrons
◦ Metallic cation is formed
Electron Sea Model
All empty space is evenly distributed v.e-
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The attraction of a metallic cation for delocalized electrons
This accounts for a lot of theproperties of metals◦ Range of melting points◦ Malleability◦ Ductile◦ Durable
Hard to remove metallic cation because of the strong e- attraction
◦ Mobile e- Explains why they are good conductors
Metallic Bonds
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Find the difference in electronegativities of the two elements
Electronegativity and Bond Type
0.5 1.7PureCovalent-share e- evenly-2 non metals and/or metalloids
Non-polar
PolarCovalent-Share e- but not evenly-One element holds e- more
Polar
Ionic-Metal and non-metal
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Count total valence electrons available
Place electrons around atoms
Ensure each atom has an octet (8)◦ Or a pair for H (2)
To create a Lewis Dot Diagram
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Draw the Lewis Structure for the molecule
Count the total number of . . .◦ Bonded regions around the central atom
DOUBLE and TRIPLE bonds count as ONE REGION◦ Unshared e- pair
Count as ONE REGION
VSEPR Rules
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Molecular Lewis Dot electron pairs around central atom
Structure structure total shared unshared
H CH4 H-C-H 4 4 0 “tetrahedral” H NH3 H-N-H 4 3 1 “trigonal H pyramidal”
H2O H-O-H 4 2 2 “bent”
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Molecule Total no. of
electron pairs
No. of shared pairs
No. of unshared pairs
Molecular shape
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A molecule is polar if◦ There is a polar bond◦ It is ASSYMETRICAL (not symmetric)
Polarity
O
HH
(-)
(+)(+)H
H
H
H
C
(+)
(+)
(+)
(+)
PolarNon-Polar
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Symmetric (non-polar)◦ Linear◦ Tetrahedral◦ Trigonal planar
If all elements around the center atom are the same
Asymmetric (polar)◦ Bent◦ Trigonal pyramidal
Typically. . .
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Van der Waals forces (London Dispersion forces)◦ Weak forces between non-polar molecules◦ These forces determine volatility
Doesn’t take much nrg to break apart (liquid gas) Most likely to be a gas
Like playing red rover and only holding pinkies together
Intermolecular Forces
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Dipole-Dipole◦ Attraction between polar molecules
Most likely to be a liquid
Play red rover and hold hands
Intermolecular Forces
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Hydrogen Bonding (H-Bonds)◦ Between hydrogen (H) and a highly
electronegative element F, O, N
◦ Extreme case of dipole-dipole◦ Strongest of the intermolecular forces
Play red rover and link elbows Needs A LOT of nrg to break bonds
Intermolecular Forces
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Carbon has a mass of 12 g
Oxygen has a mass of 16 g
H2O molecules has a mass of 18 g
How do these #’s relate to the atom or compound?◦ Atomic mass
1 mole of . . .
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Amedeo Avogadro (1776-1856) 1 mole = 6.0221415 x 1023
◦ Particles◦ Molecules◦ Atoms◦ Ions◦ Formula units◦ Etc, etc
Avogadro’s Number
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Determine the mass percentage of each element in the compound.
Percent Composition
100____
compoundofmasselementofmass
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Gives the lowest whole # ratio of elements in a compound.
The empirical formula for C6H12O6 is
The empirical formula for C2H6 is
* most basic ratio of elements in the compound
Empirical Formula
CH2O
CH3